Consider the following reaction that occurs when natural gas is burned.
CH4(g) + 2O2(g) �¨ CO2(g) + 2H2O(g)
How many moles of water are produced when 6.2 mol of methane are burned? Assume that there is more than enough oxygen present.
12
Answer is 12
Well, it seems like methane is ready to heat things up! Let's calculate the number of moles of water it'll produce.
From the balanced equation, we see that for every 1 mole of methane (CH4) burned, we get 2 moles of water (H2O) as the product.
So if we have 6.2 mol of methane, we can expect 2 times that amount of water molecules.
Therefore, 6.2 mol of methane will produce 2 * 6.2 = 12.4 mol of water.
That's enough water to make a clownfish feel right at home! 🐠😄
To determine the number of moles of water produced, we first need to use the balanced chemical equation for the reaction.
From the balanced equation: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
We see that 1 mole of methane (CH4) reacts to produce 2 moles of water (H2O).
So, for every 1 mole of methane burned, we would produce 2 moles of water.
Given that we have 6.2 moles of methane, we can use a simple proportion to find the number of moles of water produced.
Proportion:
(2 moles of water / 1 mole of methane) = (x moles of water / 6.2 moles of methane)
Cross-multiplying:
2 moles of water * 6.2 moles of methane = 1 mole of methane * x moles of water
12.4 moles of water = x moles of water
Therefore, when 6.2 moles of methane are burned, we would produce 12.4 moles of water.
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http://www.jiskha.com/science/chemistry/stoichiometry.html